1. Electron Movement and Organization 3.17.15 Objectives: Identify electron properties Understand how electrons move within an atom.

2. Characteristics of Electrons 1.What are some properties of electrons? 2.How do electrons move within an atom?

3. Electron Movement and Organization 3.18.15 Objectives: Identify electron properties Understand how electrons move within an atom.

4. Like Properties: Wavelength Wavelength: length of wave from two neighboring crest.

5. Wave-Like Properties: Frequency Wave-Like Properties: Frequency Frequency ( Hz ) : how many waves pass a certain point per second. Units: Hertz (Hz.)= (waves/second)

6. Wave-Like Properties: Energy Temperature : Represents amount of energy emitted from light particles. Photons: Light particles classified by energy emitted. *Electron movement dependent upon type of photons absorbed or released.

7. Electrons: Wave-Like Properties a. Relationship b/w wavelength and frequency? b.Relationship b/w wavelength and energy emission? c.Relationship b/w frequency and energy emission?

8. Electron Movement Electrons can take different paths around the nucleus. *Electrons constantly move to different energy levels in the electron cloud. *Direction of e- movement is dependent upon energy absorbed or released. Erwin Schrodinger

9. Electron Movement Around Nucleus A maximum of 2 electrons can move in each orbital.

11. Electron Movement Electrons can take different paths around the nucleus. *Electrons constantly move to different energy levels in the electron cloud. *Direction of e- movement is dependent upon energy absorbed or released. Erwin Schrodinger

12. Electron Movement 1.Ground state of H Atom (lowest energy level for e-) 2.A photon (light particle) is absorbed by H’s electron. Electron becomes excited and jumps to higher energy level. 3. E- returns to ground state and emits (releases) the photon. Emitted photon’s wavelength can be detected by scientists. (Infrared region at room temp; Visble region at higher temps.) 1. 2. 3.

13. Flame Test Lab Purpose: To classify atoms and identify electron movement in atoms.

15. Visible Region of EM Spectrum loke.as.arizona.edu

17. Electromagnetic Spectrum Analysis Qts.

18. Electron Movement and Organization 10.29.14 Due: E- Probability Lab(today) Nuclear Energy Qts.- typed essay (due Thurs.) Infinite Campus Update: Nuclear Energy Bell Ringer (5pts) Objectives: Understand how electrons move within atoms. Distinguish between atoms based on their different electron arrangements.

19. Electromagnetic Spectrum Analysis Qts.

20. Electromagnetic Spectrum Analysis a. Relationship b/w wavelength and frequency? b.Relationship b/w wavelength and energy emission? c.Relationship b/w frequency and energy emission?

21. Electromagnetic Spectrum Analysis a. Relationship b/w wavelength and frequency? b.Relationship b/w wavelength and energy emission? c.Relationship b/w frequency and energy emission?

22. Emission Spectrums Emission spectrum for each element is unique.

23. Electron Movement in Energy Levels Quantum of energy: Specific energy that is absorbed or emitted by electrons. Energy difference between two energy levels. Scientist can calculate energy emitted by electrons. Determine what energy levels electrons move between in an atom.

24. Locating an Electron Is it possible to know the exact location and velocity of an electron at any instant in time?

25. Locating an Electron Is it possible to know the exact location and velocity of an electron at any instant in time? Very difficult to locate an electron because: - moving extremely fast -continuously bombarded by light particles When locate an electron with a photon from a microscope, it changes its velocity in unpredictable ways.

26. Photon Before Photon changes wavelength After Heisenberg Uncertainty Principle It is not possible to know the exact position and velocity of an electron at the same time.

27. Electron Movement and Organization 3.24.15 Due: Electron Probability Lab Objectives: Understand how electrons move within atoms. Distinguish between atoms based on their different electron arrangements.

28. Electron Probability Lab ?

29. The Quantum Mechanical Model An atomic model that best explains the probable arrangement and movement of electrons at any moment in time. Schrodinger provided evidence for this model using a complex mathematical equation. Depends upon 4 quantum numbers. Erwin Schrodinger

30. n-Quantum Number n = energy levels 3-D region of space around the nucleus where an electron can be found. Each energy level has a specific energy value. E- must absorb or release a specific quantum of energy to move between energy levels. E- do not travel in an orbit (exact path) around the nucleus. Atomic orbitals: Probable paths an electron would take around the nucleus.

31. Energy Levels and the Periodic Table Associate energy levels with rows on periodic table.

32. n-Quantum Number Limited number of electrons on each energy level. 2n 2 Rule determines the maximum number of electrons on each energy level.

33. Electron Probability Lab

34. l–Quantum Number l -number : Sublevels within an energy level. Sublevels identify the shape of the orbitals. There are four different sublevels: s, p, d, f

35. Orbital Shapes A maximum of 2 electrons can move in each orbital.

36. Orbitals and Energy Requirement Electron movement defines orbital shapes for each sublevel. Electrons need energy to move in orbital shapes. Sublevel’s OrbitalsEnergy for electron movement (Rank in increasing amount of energy) S-orbital P-orbital D-orbital F-orbital

37. Electron Configuration Electron Configuration: The probable arrangement of electrons in the ground state of an atom. Electron Configuration Rules: Aufbau Principle: Electrons will move in an orbital of lower energy first. (Electrons are lazy!) Pauli Exclusion Principle: Only two electrons can move in an orbital at the same time. Hund’s Rule: When electrons can move in orbitals of the same energy, they will prefer to be alone before pairing up. (Electrons are selfish!)

38. Electron Movement and Organization 3.25.15 Due: Electron Probability Lab Objectives: Understand how electrons move within atoms. Distinguish between atoms based on their different electron arrangements.

39. Bell Ringer: Electron Arrangement 1. What atomic model best explains electron arrangement? 2. a. What is the n-quantum number? b. T or F: Electron move around the nucleus in an exact path. 3. a. What is the l-quantum number? b. Illustrate the s, p, d, f atomic orbitals? c. How many electrons can move in each atomic orbital at any one time?

40. Orbital Shapes A maximum of 2 electrons can move in each orbital.

41. Orbitals and Periodic Table

43. Bell Ringer: Electron Arrangement 1. What atomic model best explains electron arrangement? 2. a. What is the n-quantum number? b. T or F: Electron move around the nucleus in an exact path. 3. a. What is the l-quantum number? b. Illustrate the s, p, d, f atomic orbitals? c. How many electrons can move in each atomic orbital at any one time?

44. Electron Configuration

47. Electron Configuration: Bell Ringer 1.What is electron configuration for an element? 2. How does the periodic table help you determine electron configuration for an element? Be specific with your explanation.

48. Electron Sublevels (atomic orbitals) Diagonal Rule 3. Use the diagram to determine the type of sublevels (orbitals) in each energy level? 1 st : 2 nd : 3 rd : 4 th : 5 th : 6 th : 7 th : 2. What do you suppose the yellow arrows represent? khanacademy.org

49. Periodic Table and Electron Configuration

50. Orbital Shapes A maximum of 2 electrons can move in each orbital.

51. Electron Configuration: Exit Slip Br: Ar: Fe

54. Electron Configuration Electron Configuration: The probable arrangement of electrons in the ground state of an atom. Electron Configuration Rules: Aufbau Principle: Electrons will move in an orbital of lower energy first. (Electrons are lazy!) Pauli Exclusion Principle: Only two electrons can move in an orbital at the same time. Hund’s Rule: When electrons can move in orbitals of the same energy, they will prefer to be alone before pairing up. (Electrons are selfish!)

55. m- Quantum Number m –number: Orientations for each atomic orbital. Orbital orientations: The different ways an electron can make an orbital in 3-D space.

56. S-Orbital Orientation Maximum # of s-orbital electrons on an energy level? How many s-orbital orientations are possible on an energy level?

59. P-orbital Orientations Maximum # of p-orbital electrons on an energy level? How many p-orbital orientations are possible on an energy level?

61. D-orbital Orientations Maximum # of d-orbital electrons on an energy level? How many d-orbital orientations are possible on an energy level?

63. F-orbital Orientations Maximum # of f-orbital electrons on an energy level? How many f-orbital orientations are possible on an energy level?

65. Orbital Orientations

66. Electron Movement and Organization 11.05.14 Infinite Campus: Electron Probability Lab (15pts.) Objectives: Understand how electrons move within atoms Distinguish between atoms based on their different electron arrangements.

67. Electron Configuration with orbital notation 1. Define the first three quantum numbers. 2. Write the electron configuration (n,l,m quantum numbers) for each element below: H: Li: C: V:

68. Electron Configuration Orbital Notation

69. S-Quantum Numbers S-number : The direction an electron spins in an orbital. If paired, the electrons will spin in opposite directions.

70. Electron Configuration: Bell Ringer Electron Configuration: Bell Ringer 1.a. Determine the electron configuration of a neutral Br atom and include the orbital notations. b. How many unpaired electrons? c. How many valence electrons does Br have? d. How many types of sublevels (orbitals) use Hund’s rule?

71. Orbitals and Periodic Table

72. Nuclear Chemistry and Electron Arrangement Exam

73. Balancing Redox Reactions: Acidic Solutions Cu (s) + NO 3 - (aq) ----> Cu 2+ (aq) + NO 2 (g)